Given the reaction: P₄(l) + 6 Cl₂(g) → 4 PCl₃(l)
If the percent yield is 82%, what mass of P⁴ is required to obtain 2.30 g PCl₃ (Cl₂ in excess) ?

Question

Given the reaction: P₄(l) + 6 Cl₂(g) → 4 PCl₃(l) If the percent yield is 82%, what mass of P⁴ is required to obtain 2.30 g PCl₃ (Cl₂ in excess)?

Quizplus · Accepted Answer

The balanced equation is: P₄(l) + 6 Cl₂(g) → 4 PCl₃(l)From the stoichiometry, we can see that 1 mole of P₄ reacts with 6 moles of Cl₂ to produce 4 moles of PCl₃.The molar mass of P₄ is 123.9 g/mol, and the molar mass of PCl₃ is 137.3 g/mol.Therefore, 123.9 g of P₄ will react with 6 moles of Cl₂ to produce 4 moles of PCl₃, which is 549.2 g of PCl₃.If the percent yield is 82%, then the actual yield of PCl₃ will be 0.82 * 549.2 g = 451.3 g.To obtain 2.30 g of PCl₃, we need to use (2.30 g / 451.3 g) * 123.9 g = 0.63 g of P₄.

Given the Reaction: P4(l) + 6 Cl2(g) → 4 PCl3(l)

Given the Reaction: P₄(l) + 6 Cl₂(g) → 4 PCl₃(l)